Domanda del libro di testo
Molybdenum (mp 2623 °C) has a higher melting point than yttrium (mp 1522 °C) or cadmium (mp 321 °C). Explain.
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Ch.21 - Transition Elements and Coordination Chemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblema 42
McMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblema 42Capitolo 21, Problema 42
Briefly account for each of the following observations:
(a) Atomic radii decrease in the order Sc > Ti > V.
(b) Densities increase in the order Ti > V > Cr.
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Understand the periodic trends and how they affect atomic radii and density. Atomic radii generally decrease across a period from left to right due to the increase in nuclear charge which pulls the electrons closer to the nucleus.
Examine the position of Scandium (Sc), Titanium (Ti), and Vanadium (V) in the periodic table. They are located in the same period with increasing atomic number. This increase in atomic number from Sc to V means an increase in the effective nuclear charge, explaining the decrease in atomic radii.
Consider the factors affecting density, which include atomic mass and volume. As atomic number increases, generally so does the mass. However, the volume can decrease if the atomic radius decreases.
Analyze the positions of Titanium (Ti), Vanadium (V), and Chromium (Cr) in the periodic table. They are consecutive elements in a period, and as you move from Ti to Cr, the atomic mass increases while the atomic radius decreases, leading to an increase in density.
Relate the increase in nuclear charge with the decrease in atomic radius and the increase in density. The stronger nuclear pull (higher nuclear charge) as you move from Sc to V and from Ti to Cr not only decreases the atomic radius but also increases the density due to a smaller volume occupied by the atoms.
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Atomic Radius Trends
Atomic radius refers to the size of an atom, typically measured from the nucleus to the outermost electron shell. As you move across a period in the periodic table from left to right, atomic radii generally decrease due to increased nuclear charge, which pulls electrons closer to the nucleus. In the case of Sc, Ti, and V, the decrease in atomic radius can be attributed to the increasing positive charge in the nucleus as you move from Sc to V.
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01:42
Atomic Radius Trends
Density and Atomic Mass
Density is defined as mass per unit volume and is influenced by both the mass of the atoms and how closely they are packed in a given volume. As you move from Ti to V to Cr, the densities increase due to the increase in atomic mass and the arrangement of atoms in the crystal lattice. The transition metals exhibit varying densities based on their atomic structure and bonding characteristics.
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02:19Atomic Mass
Transition Metals and Electron Configuration
Transition metals, such as Sc, Ti, V, and Cr, have unique electron configurations that affect their physical properties, including atomic radius and density. The presence of d-electrons contributes to the complexity of their bonding and packing in solid form. Understanding how these electrons influence the size and mass of the atoms helps explain the observed trends in atomic radii and densities among these elements.
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00:53Electron Configurations Of Transition Metals Example
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